Explanation The equilibrium reaction is given below. C H 3 N H 2 ( a q ) + H 2 O ( l ) ⇌ C H 3 N H 3 + ( a q ) + O H − ( a q ) The base ionization constant can be written as given below. K b = [ C H 3 N H 3 + ] [ O H − ] [ C H 3 N H 2 ] A table can be set up as shown below. C H 3 N H 2 ( a q ) O H − ( a q ) C H 3 N H 3 + ( a q ) I n i t i a l c o n c . ( M ) 0.024 1 × 10 − 7 0 C h a n g e i n c o n c . ( M ) − x + x + x E q u i l i b r i u m c o n c . ( M ) 0.024 − x x x The concentration of O H − comes from its autoionization that is 1.0 × 10 − 7 . It is assumed to be small compared to the change. At equilibrium, K b = ( x ) ( x ) ( 0

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ISBN: 9781285199047

Author: John W. Moore, Conrad L. Stanitski

Publisher: Cengage Learning

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Chapter 14, Problem 61QRT

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Interpretation:

The pH and [OH−] of a 0.024 M aqueous solution of methyl amine has to be calculated.

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Chapter 14, Problem 60QRT

Chapter 14, Problem 62QRT

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The p H and [ O H − ] of a 0.024 M aqueous solution of methyl amine has to be calculated.

Solution Summary: The author calculates the pH and the left[OH-right] of a 0.024M solution. The equilibrium reaction is given below.

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Interpretation:

The pH and [OH−] of a 0.024 M aqueous solution of methyl amine has to be calculated.

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Chapter 14 Solutions

The p H and [ O H − ] of a 0.024 M aqueous solution of methyl amine has to be calculated.

Solution Summary: The author calculates the pH and the left[OH-right] of a 0.024M solution. The equilibrium reaction is given below.

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Interpretation: The pH and [OH−] of a 0.024 M aqueous solution of methyl amine has to be calculated.

Want to see the full answer?

Chapter 14 Solutions

Interpretation:

The pH and [OH−] of a 0.024 M aqueous solution of methyl amine has to be calculated.